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and non-polar species. In many cases, they have been found to perform much better than commonly used solvents. P erhaps the m ost i ntriguing feature of these compounds is that, while they a re liquid in t heir pure state at or near room temperature, they have essentially no vapor pressure. They do not evaporate, and so they cannot lead to fugitive emissions. Many of these compounds are liquids over incredibly large temperature ranges, from below ambient to well over 300 to 400 oC, which suggests they could be used under unique CO2 processing conditions [33-35]. For use in CO2 separations, the tunability of ILs is invaluable. There are virtually endless possibilities for cations, anions, substituents, and functional groups that can be incorporated into ILs. As a result, there are i nnumerable c ombinations pos sible, pr oviding t he oppor tunity t o opt imize phy sical a nd c hemical properties for specific applications like CO2 capture. Figure 7. Phase diagram of CO2 with 1-butyl-3-methylimidazolium hexafluorophosphate [36]. The solubility of CO2 in an ionic liquid was first measured in 1999 [35], as shown in Figure 7. The discovery that CO2 had significant solubility within ILs led to the idea of using ILs as a sorbent for separating CO2 from other gases [37]. 0.035 0.030 0.025 0.020 0.015 0.010 0.005 0.000 N2 O2 CO2 CH4 C2H6 C2H4 Solvent Figure 8. Solubility of CO2 in various solvents at a partial pressure of 1 atm and temperature of 298.15 K [38]. Carbon Capture Factual Document 22 Mole Fraction of Gas Heptane Cyclohexane Benzene Methanol Ethanol Acetone hmpy Tf2N hmim Tf2NPDF Image | 2020 Carbon Capture
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